Now that you have tried the simulation answer the following questions. 1. When you pull clothes out of the dryer, sometimes they stick together. What do you think might explain why they stick? 2. What do you think happens in the dryer that makes the clothes stick together?
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- 5.0 g of brass (Cp = 0.38 J/g-oC, initially at 68oC) and 3.5 g of aluminum (Cp = 0.9 J/g-oC, initially at 83oC) are dropped into 20 g of water (Cp = 4.184 J/g-oC, initially at 23oC). Based on the described system, which of the following statements is/are correct? Check all that apply. Brass will release heat. Aluminum will release heat. Water will absorb heat. Air will absorb heat.Calculate the amount of heat needed to boil 117.g of benzene (C6H6), beginning from a temperature of 43.8°C. Be sure your answer has a unit symbol and the correct number of significant digits. Pls help and explain how did you get to the answer asap!During a recent winter month in Sheboygan, Wisconsin, it was necessary to obtain 3500 kWh of heat provided by a natural gas furnace with 89% efficiency to keep a small house warm (the efficiency of a gas furnace is the percent of the heat produced by combustion that is transferred into the house). (a) Assume that natural gas is pure methane and determine the volume of natural gas in cubic feet that was required to heat the house. The average temperature of the natural gas was 56 °F; at this temperature and a pressure of 1 atm, natural gas has a density of 0.681 g/L. (b) How many gallons of LPG (liquefied petroleum gas) would be required to replace the natural gas used? Assume the LPG is liquid propane [C3H8: density, 0.5318 g/mL; enthalpy of combustion, 2219 kJ/mol for the formation of CO2(g) and H2O(l)] and the furnace used to burn the LPG has the same efficiency as the gas furnace. (c) What mass of carbon dioxide is produced by combustion of the methane used to heat the house? (d)…
- You pour a cup of tea that has a volume of 128 mL and is initially 92.1 °C. You place a stainless steel spoon that has a mass of 42.13 g and a temperature of 20.92 °C into the coffee. What is the final temperature °C of the coffee and spoon at thermal equilibrium assuming no heat is lost to the surroundings? Assume the specific heat and density of coffee to be the same as water. The specific heat of the spoon is 0.466 J/g·°C. Report your answer normallly to one decimal place and do not include units.Introduction: For this experiment, 16.55 grams of nitrogen gas and 10.15 grams of hydrogen gas are allowed to react in the reaction vessel. The ammonia vapor that is produced is then condensed, liquefied, and collected into a collection vessel. 1. Write a balanced thermochemical equation with phase labels for the Haber process with the heat energy as part of the equation.The current US debt as of 1/10/23 was approximately 31.5 trillion (31,500,000,000). Calculate how far a stack on dollar bills in this amount would reach in miles. Show work.
- Most people find waterbeds uncomfortable unless the water temperature is maintained at about 85 °F. Unless it is heated, a waterbed that contains 892 L of water cools from 85 °F to 72 °F in 24 hours. Estimate the amount of electrical energy required over 24 hours, in kWh, to keep the bed from cooling. Note that 1 kilowatt-hour (kWh) = 3.6 × 106 J, and assume that the density of water is 1.0 g/mL (independent of temperature). What otherassumptions did you make? How did they affect your calculated result (i.e., were they likely to yield “positive” or “negative” errors)?9.16 According to Figure 9.2, the total energy supply in the United States in 2016 was 111.261015 Btu. Express this value in joules and in calories. FIGURE 9.2 Energy production and consumption (in quadrillion Btu) in the United States during the year 2016. The discussion in the text explains how to read this complex figure, which contains an enormous amount of information about the energy economy. Data come from the Department of Energy and do not always add up exactly as expected due to rounding and other issues.During a recent winter month in Sheboygan, Wisconsin, it was necessary to obtain 3500 kWh of heat provided by a natural gas furnace with 89% efficiency to keep a small house warm (the efficiency of a gas furnace is the percent of the heat produced by combustion that is transferred into the house). (a) Assume that natural gas is pure methane and determine the volume of natural gas in cubic feet that was required to heat the house. The average temperature of the natural gas was 56 F; at this temperature and a pressure of 1 atm, natural gas has a density of 0.68 1 g/L. (b) How many gallons of LPG (liquefied petroleum gas) would be required to replace the natural gas used? Assume the LPG is liquid propane [ C3H8 : density, 0.5318 g/mL; enthalpy of combustion, 2219 Id/mo for the formation of CO2(g) and H2O(l) ] and the furnace used to burn the LPG has the same efficiency as the gas furnace. (c) What mass of carbon dioxide is produced by combustion of the methane used to heat the house? (d) What mass of water is produced by combustion of the methane used to heat the house? (e) What volume of air is required to provide the oxygen for the combustion of the methane used to heat the house? Air contains 23% oxygen by mass. The average density of air during the month was 1.22 g/L. (f) How many kilowatt—hours ( 1kWh=3.6106 J) of electricity would be required to provide the heat necessary to heat the house? Note electricity is 100% efficient in producing heat inside a house. (g) Although electricity is 100% efficient in producing heat inside a house, production and distribution of electricity is not 100% efficient. The efficiency of production and distribution of electricity produced in a coal-fired power plant is about 40%. A certain type of coal provides 2.26 kWh per pound upon combustion. What mass of this coal in kilograms will be required to produce the electrical energy necessary to heat the house if the efficiency of generation and distribution is 40%?
- Ethylene glycol is the main component in automobile anti-freeze. To monitor the temperature of an auto cooling system, you intend to use a meter that reads from 0 to 100. You devise a new temperature scale based on the approximate melting and boiling points of a typical antifreeze solution (45C and 115C). You wish these points to correspond to 0A and 100A, respectively. a. Derive an expression for converting between A and C. b. Derive an expression for converting between F and A. c. At what temperature would your thermometer and a Celsius thermometer give the same numerical reading? d. Your thermometer reads 86A. What is the temperature in C and in F? e. What is a temperature of 45C in A?A student is given a sample of a pink manganese (II) chloride hydrate. She weighs the sample in a dry, covered crucible and obtains a mass of 26.742g for the crucible, cover, and sample. Earlier she had found that the crucible and cover weighed 23.599g. She then heats the crucible to drive off the water of hydration, keeping the crucible at red heat for about 10 minutes with the cover slightly ajar. She then lets the crucible cool and finds it has a lower mass; the crucible, cover and contents then weigh 25.598g. In the process the sample was converted to off-white anhydrous MnCl2. a. What was the mass of the hydrate sample? _ghydrate b. What is the mass of the anhydrous MnCl2? _gMnCl2 c. How much water was driven off? _gH2O d. What is the percent by mass of water in the hydrate? water=massofwaterinsamplemassofhydrateinsample100 _massH2O e. How many grams of water would there be in 100.0g hydrate? How many moles? _gH2O; _molesH2O f. How many grams of MnCl2 are there in 100.0g hydrate? How many moles? What percentage of the hydrate is MnCl2? Convert the mass of MnCl2 to moles. The molar mass of MnCl2 is 125.85g/mol. _gMnCl2; _molesMnCl2 g. How many moles of water are present per mole MnCl2? _ h. What is the formula of the hydrate? _You have the six pieces of metal listed below, plus a beaker of water containing 3.00 102 g of water. The water temperature is 21.00 C. (a) In your first experiment you select one piece of metal and heat it to 100 C, and then select a second piece of metal and cool it to 10 C. Both pieces of metal are then placed in the beaker of water and the temperatures equilibrated. You want to select two pieces of metal to use, such that the final temperature of the water is as high as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water? (b) The second experiment is done in the same way as the first. However, your goal now is to cause the temperature to change the least, that is, the final temperature should be as near to 21.00 C as possible. What piece of metal will you heat? What piece of metal will you cool? What is the final temperature of the water?